S(s)+32O2(g)→SO3(g)+2x K.calSO2(g)+12O2(g)→SO3(g)+y K.calWhich would be the enthalpy of formation of SO2?

S+32O2→SO3 ΔH=−2x k.cal→(1) SO2+12O2→SO3 ΔH=−y k.cal→(2) (1)−(2) S+O2→SO2 ΔH=y−2x

S(s)+32O2(g)→SO3(g)+2x K.calSO2(g)+12O2(g)→SO3(g)+y K.calWhich would be the enthalpy of formation of SO2?

S+32O2→SO3 ΔH=−2x k.cal→(1) SO2+12O2→SO3 ΔH=−y k.cal→(2) (1)−(2) S+O2→SO2 ΔH=y−2x

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$\underset{(s)}{S} + \frac{3}{2} \underset{(g)}{O_{2}} \to \underset{(g)}{S O_{3}} + 2 x K . c a l$
$\underset{(g)}{S O_{2}} + \frac{1}{2} \underset{(g)}{O_{2}} \to \underset{(g)}{S O_{3}} + y K . c a l$
Which would be the enthalpy of formation of $S O_{2}$ ?

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$2 x - y$

$2 x + y$

$y - 2 x$

$\frac{2 x}{y}$

answer is C.

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$S + \frac{3}{2} O_{2} \to S O_{3} Δ H = - 2 x k . c a l \to (1)$

$S O_{2} + \frac{1}{2} O_{2} \to S O_{3} Δ H = - y k . c a l \to (2)$

$(1) - (2) S + O_{2} \to S O_{2} Δ H = y - 2 x$

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S(s)+32O2(g)→SO3(g)+2x K.calSO2(g)+12O2(g)→SO3(g)+y K.calWhich would be the enthalpy of formation of SO2?

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$\underset{(s)}{S} + \frac{3}{2} \underset{(g)}{O_{2}} \to \underset{(g)}{S O_{3}} + 2 x K . c a l$
$\underset{(g)}{S O_{2}} + \frac{1}{2} \underset{(g)}{O_{2}} \to \underset{(g)}{S O_{3}} + y K . c a l$
Which would be the enthalpy of formation of $S O_{2}$ ?